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3 years ago

What are the reactants found in soap and detergents?

Chemistry

2 answers:

babymother [125]3 years ago

8 0

https://www.britannica.com/science/soap/Raw-materials

Leni [432]3 years ago

7 0

NaOH. I'm pretty sure thats the chemical equation for Lye. SO.. Hope that helps at all. :)

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How much heat must be removed from 456 g of water at 25. 0 c to hcange it into ice at 10 c

ValentinkaMS [17]

The heat required to convert water is given as the product of the mas and the latent heat. 28.34 kJ heat must be removed from the water to change it into ice.

<h3>What is heat energy?</h3>

Heat energy is the product of mass, specific heat capacity, and temperature change. It is given as,

$\rm Q = mc \Delta T$

Given,

Mass of water = 456 gm

Specific heat capacity = 4.186 J / g K

Temperatutre change = 14.85 K

Substituting values above:

$\begin{aligned} \rm Q &= 456 \times 4.186 \times 14.85\\\\&= 28345.91\;\rm J\\\\&= 28.34\;\rm kJ\end{aligned}$

Therefore, 28.34 kJ of heat energy should be removed from the water.

Learn more about the heat here:

brainly.com/question/14052023

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2 years ago

Atomic Size: Determine which of the following element pairs is the larger one

aleksklad [387]

Answer: I think the answer is 3.) Krypton or Argon.

Explanation:

4 0

3 years ago

For the following reaction, 4.31 grams of iron are mixed with excess oxygen gas . The reaction yields 5.17 grams of iron(II) oxi

natka813 [3]

<u>Answer:</u> The theoretical yield of iron (II) oxide is 5.53g and percent yield of the reaction is 93.49 %

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ ....(1)

<u>For Iron:</u>

Given mass of iron = 4.31 g

Molar mass of iron = 53.85 g/mol

Putting values in above equation, we get:

$\text{Moles of iron}=\frac{4.31g}{53.85g/mol}=0.0771mol$

For the given chemical reaction:

$2Fe(s)+O_2(g)\rightarrow 2FeO(s)$

By Stoichiometry of the reaction:

2 moles of iron produces 2 moles of iron (ii) oxide.

So, 0.0771 moles of iron will produce = $\frac{2}{2}\times 0.0771=0.0771mol$ of iron (ii) oxide

Now, calculating the theoretical yield of iron (ii) oxide using equation 1, we get:

Moles of of iron (II) oxide = 0.0771 moles

Molar mass of iron (II) oxide = 71.844 g/mol

Putting values in equation 1, we get:

$0.0771mol=\frac{\text{Theoretical yield of iron(ii) oxide}}{71.844g/mol}=5.53g$

To calculate the percentage yield of iron (ii) oxide, we use the equation:

$\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100$

Experimental yield of iron (ii) oxide = 5.17 g

Theoretical yield of iron (ii) oxide = 5.53 g

Putting values in above equation, we get:

$\%\text{ yield of iron (ii) oxide}=\frac{5.17g}{5.53g}\times 100\\\\\% \text{yield of iron (ii) oxide}=93.49\%$

Hence, the theoretical yield of iron (II) oxide is 5.53g and percent yield of the reaction is 93.49 %

7 0

3 years ago

What is the most important monosaccharide on Earth?

Lelechka [254]

Answer:

the answer is A Glucose

hope it helps!

6 0

3 years ago

1362205.2 in scientific notation

SVETLANKA909090 [29]

1.3622052x10^6 you move the . 6 places to the left making it a positive 10^6

8 0

3 years ago